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AP 2 Modern Physics

Total questions: 36

Worksheet time: 1hrs 8mins

Name
Class
Date
1.
Light of a single wavelength is incident on a metal.  Electrons are released. The intensity of the light is then increased.
Which of the following changes occur?
a)
Rate of electron emission: increase.
Energy of electrons: increase.
b)
Rate of electron emission: decrease.
Energy of electrons: no change.
c)
Rate of electron emission: decrease.
Energy of electrons: increase.
d)
Rate of electron emission: increase.
Energy of electrons: no change.
2.
The photoelectric effect only occurs if the light shining on the metal is:
a)
coherent.
b)
above a minimum intensity.
c)
above a minimum frequency.
d)
above a minimum wavelength.
3.
The graph shows maximum kinetic energy of emitted electrons against frequency of incident light for a number of different metals.
Plank's constant is determined by:
a)
the x-intercept.
b)
the y-intercept.
c)
the gradient.
d)
the area under the graph.
4.
The graph shows maximum kinetic energy of emitted electrons against frequency of incident light for a number of different metals.
The threshold frequency is determined by:
a)
the x-intercept.
b)
the y-intercept.
c)
the gradient.
d)
the area under the graph.
5.
Which statement about the photoelectric effect is correct?
a)
Electrons are emitted instantaneously.
b)
Electrons are not emitted below a certain wavelength.
c)
You can change the energy of the electrons by changing the intensity.
d)
Electron energy is independent of frequency.
6.
The photoelectric effect is when:
a)
Electrons collide inside a metal to release photons.
b)
One incident metal electron releases one photon.
c)
One incident photon releases one electron from a metal.
d)
Photons are absorbed in to metal ions releasing electrons.
7.
What is the maximum kinetic energy of electrons emitted from cesium (Cs), when light of frequency1015 Hz falls upon the metal? (work function for Cs is 1.8 eV)
a)
7.728x10-19 J
b)
4.83 eV
c)
1.864x10-19 J
d)
2.34 eV
8.
Does high-frequency or low frequency light cause the ejection of a greater number of electrons from a metal surface?
a)
only high frequency
b)
only low frequency
c)
both of them
d)
doesn't depend to frequency
9.
Do the photons of violet light or the photons of red light, falling on a metal surface with the same intensity,cause emission of more electrons?
a)
 red light
b)
violet light
c)
same 
10.
The cut-off wavelength for the photoelectric effect of platinum is 220 nm. Find the work function of platinum in eV
a)
11.25 eV
b)
9 eV
c)
4.5 eV
d)
5.65 eV
11.
Find the cut-off wavelength for the photoelectriceffect in tungsten (work function for tungsten is 4.5 eV)
a)
138 nm
b)
414 nm
c)
552 nm
d)
276 nm
12.
Green light with a wavelength of 5461 Å, emitted from a mercury lamp, ejects photoelectrons with a maximum kinetic energy of 0.13 eV from a metal surface. Calculate the work function of the metal.
a)
2.14 eV
b)
1.07 eV
c)
3.21 eV
d)
0.535 eV
13.
Green light with a wavelength of 5461 Å, emitted from a mercury lamp, ejects photoelectrons with a maximum kinetic energy of 0.13 eV from a metal surface.Calculate the cut-off wavelength of the metal
a)
290 nm
b)
580 nm
c)
145 nm
d)
435 nm
14.
The diagram shows a circuit involving a photoelectric cell. When UV light is shone onto the metal cathode, electrons are emitted establishing a photocurrent.
Which of the following changes could cause the photocurrent to stop?
a)
Increasing the potential difference of the power supply.
b)
Increasing the frequency of the UV light.
c)
Increasing the intensity of the UV light.
d)
Changing the metal surface to one with a smaller work function.
15.
The photoelectric effect helps us to understand
a)
the particle nature of light.
b)
diffraction pattern produced as light passes through a single slit.
c)
the wave behavior of light.
d)
spectroscopes.
16.
This image is an illustration of
a)
photoelectric effect
b)
Dalton's atomic theory
c)
Bohr model
d)
Quantum mechanical model
17.

All particles have momentum, even particles with no mass. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

18.

Energy at the atomic level (microscopic) can only exist in specific amounts. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

19.

When light of specific frequencies is shined on a surface, electrons are ejected from the surface. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

20.

If waves can behave like particles, then particles can behave like a wave. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

21.

A person cannot measure the location and the speed (momentum) of an object at the same time. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

22.

Which famous experiment showed up what the inside of an atom was like?

a)

Gold Foil Experiment

b)

Double Slit Experiment

c)

Oil Drop Experiment

d)

Schrodinger's Cat Experiment

23.

What did Einstein win his Nobel Prize for?

a)

E = mc2

b)

Special Relativity

c)

General Relativity

d)

Photoelectric Effect

24.

Why do we see colors when we look at neon signs?

a)

Electrons are jumping from an excited state to a normal state and giving off energy

b)

Electrons are jumping from a normal state to an excited state and absorbing energy

c)

Electrons are jumping from an excited state to a normal state and absorbing energy

d)

Electrons are jumping from a normal state to an excited state and giving off energy

25.

Which equation is used to calculate the wavelength associated with matter?

a)

c = λν

b)

λ = c/ν

c)

λ = h / mv

d)

λ = ch / E

26.
How is the Quantum Mechanical Model different from Bohr's planetary model?
a)
The QMM shows the probability of the electron's location.
b)
The planetary model shows the probability of the electron's location.
c)
The QMM shows the exact location of the electron. 
d)
The QMM does not include a nucleus.
27.

The atomic number represents:

a)

protons + neutrons

b)

protons

c)

neutrons

d)

electrons + neutrons

28.

Which scientist discovered that electrons move outside the nucleus in orbitals within a cloud?

a)

N. Bohr

b)

J. Chadwick

c)

E. Schrodinger

d)

L. DeBroglie

29.
Which scientist concluded that the atom is mostly empty space?
a)
E. Rutherford
b)
N. Bohr
c)
JJ. Thomson
d)
J. Dalton
30.

Which scientist thought electrons moved in orbits like planets circling the sun?

a)

J. Dalton

b)

N. Bohr

c)

L. DeBroglie

d)

R. Milliken

31.

Which scientist is famous for his oil drop experiment and eventually discovering the size of the charge on an electron and the mass of the electron?

a)

J. Chadwick

b)

R. Milliken

c)

J. Dalton

d)

N. Bohr

32.

Which scientist is responsible for discovering that most of the mass of the atom is centrally located and is positively charged?

a)

J. Chadwick

b)

N. Bohr

c)

JJ Thomson

d)

E. Rutherford

33.

Which scientist thought the atom looked like plum pudding?

a)

J. Dalton

b)

E. Schrodinger

c)

N. Bohr

d)

JJ Thomson

34.

All of the following are true of Isotopes of a certain element EXCEPT:

a)

different number of neutrons

b)

different mass numbers

c)

different atomic numbers

d)

different atomic masses

35.

Which scientist used the Gold Foil experiment to help him discover the atom is mostly empty space?

a)

W. Heisenberg

b)

E Rutherford

c)

R. Milliken

d)

J. Chadwick

36.

In his experiment, Rutherford concluded that atoms have a nucleus because

a)

most of the particles went straight through the foil.

b)

some of the particles were deflected near the front of the screen.

c)

some of the particles were deflected back towards the alpha source.

d)

not enough information is given.

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